Balance the following equation- H2CO2 - KMnO4 - CO2 - K2O - MnO

The correct option is A 5H_2CO_2 + 2KMnO_4 → 5CO_2 + K_2O + 2MnO+5H_2O The unbalanced redox equation is as follows: H_2CO_2 + KMnO_4 → CO_2 + K_2O + M ...

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Byju's Answer

Standard XII

Chemistry

Stoichiometric Calculations

Balance the f...

Question

Balance the following equation:

$H_{2} C O_{2} + K M n O_{4} \to C O_{2} + K_{2} O + M n O$

5 H_{2} C O_{2} + 2 K M n O_{4} \to 5 C O_{2} + K_{2} O + 2 M n O + 5 H_{2} O

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5 H_{2} C O_{2} + 3 K M n O_{4} \to 5 C O_{2} + 5 K_{2} O + 3 M n O + 5 H_{2} O

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3 H_{2} C O_{2} + K M n O_{4} \to 5 C O_{2} + 3 K_{2} O + 2 M n O + 5 H_{2} O

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Solution

The correct option is A $5 H_{2} C O_{2} + 2 K M n O_{4} \to 5 C O_{2} + K_{2} O + 2 M n O + 5 H_{2} O$
The unbalanced redox equation is as follows:
$H_{2} C O_{2} + K M n O_{4} \to C O_{2} + K_{2} O + M n O$
Balance all atoms other than H and O.
$H_{2} C O_{2} + 2 K M n O_{4} \to C O_{2} + K_{2} O + 2 M n O$
The oxidation number of Mn changes from +7 to 2. The change in the oxidation number of Mn is 5. Total change for 2 Mn aoms is 10.
The oxidation number of C changes from +2 to +4. The change in the oxidation number is 2.
The increase in the oxidation number is balanced with decrease in the oxidation number by multiplying $H_{2} C O_{2}$ and $C O_{2}$ with 5.
$5 H_{2} C O_{2} + 2 K M n O_{4} \to 5 C O_{2} + K_{2} O + 2 M n O$
O atoms are balanced by adding 5 water molecules on RHS.
$5 H_{2} C O_{2} + 2 K M n O_{4} \to 5 C O_{2} + K_{2} O + 2 M n O + 5 H_{2} O$
This is the balanced chemical equation.

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Similar questions

Q. The stoichiometric coefficient

n

in the following reaction is :

n H_{2} C O_{2} + 2 K M n O_{4} \to n C O_{2} + K_{2} O + 2 M n O + H_{2} O

Q. Which of the following reactions are disproportionation reactions?
(I)

C u^{+} \to C u^{2 +} + C u

(II)

3 M n O_{4}^{-} + 4 H^{+} \to 2 M n O_{4}^{-} + M n O_{2} + 2 H_{2} O

(III)

2 K M n O_{4} \to K_{2} M n O_{4} + M n O_{2} + O_{2}

(IV)

2 M n O_{4}^{-} + 3 M n^{2 +} + 2 H_{2} O \to 5 M n O_{2} + 4 H^{+}

K M n O_{4}

(mol. Wt

= 158

) oxidizes acid in acidic medium to

C O_{2}

and water as follows.

5 C_{2} O_{4}^{2 -} + 2 M n O^{-} + 16 H^{+} \to 10 C O_{2} + 2 M n^{2 +} + 8 H_{2} O

What is the equivalent weight of

K M n O_{4}

Q. Identify the correctly balanced redox reaction using ion-electron method.

F e S O_{4} + K M n O_{4} + H_{2} S O_{4} \to F e_{2} (S O_{4})_{3} + M n S O_{4} + H_{2} O + K_{2} S O_{4}

Which of the following are the products formed on heating $C u S O_{4} . 5 H_{2} O (s)$ ?

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Balance the following equation:H2CO2+KMnO4→CO2+K2O+MnO

Balance the following equation:

$H_{2} C O_{2} + K M n O_{4} \to C O_{2} + K_{2} O + M n O$